Liquids MCQs with Answers
Why does CHCl₃ (Chloroform) exist in a liquid state?
Dipole-dipole and London dispersion forces
Dipole-induced dipole forces
Hydrogen bonding
dipole-dipole forces
Which of the following has the highest boiling point?
The dominant Van der Waals force in NH₃ is:
London dispersion forces
Dipole-induced dipole forces
Dipole-dipole forces
Hydrogen bonding
Liquids have no definite shape because:
The intermolecular forces in liquids are weaker than in solids
Liquid molecules have kinetic energy less than gases
All statements are correct
The molecules of liquid are in constant motion, sliding over each other
Why is propanone (acetone) miscible in water?
Both are polar molecules
Hydrogen bonding occurs between them
Dipole-dipole attraction exists between them
All of these
Strong dipole-dipole forces among liquid molecules are responsible for:
Very low boiling point
Very low heat of vaporization
All are correct
Very high heat of vaporization
Which of the following is the correct order of increasing intermolecular interactions?
Hydrogen bonding, London forces, Dipole-dipole
London forces, Hydrogen bonding, Dipole-dipole
Dipole-dipole, London forces, Hydrogen bonding
London forces, Dipole-dipole, Hydrogen bonding
Which of the following has the strongest intermolecular forces?
Hydrogen (H₂)
Chlorine (Cl₂)
Methane (CH₄)
Iodine (I₂)
What type of force exists between ions and water molecules?
Dipole-induced dipole forces
Dipole-dipole forces
London dispersion forces
Ion-dipole forces
Which forces are present between all types of atoms and molecules?
Hydrogen bonding
Dipole-dipole forces
Dipole-induced dipole forces
London dispersion forces
The attractive forces between the partial positive end of one molecule and the partial negative end of another molecule are called:
Ion-dipole forces
London dispersion forces
Debye forces
Dipole-dipole forces
Why do liquids take the shape of their container?
Liquids do not have a definite volume
Liquids are highly compressible
Liquid molecules can slide over each other
Liquids do not have a definite shape
Nature of bonding affects the properties like:
Solubility
Melting, boiling points and isomerism
Reaction kinetics
All of these
Vapour pressure of water at 0°C is 4.579 torr, and at 10°C it is 9.209 torr, so increase in vapour pressure from 0 C to 10 C is 4.630 torr What will be the change in vapour pressure from 90°C to 100°C?
4.630 torr
< 4.630 torr
v.p remains same at all temperatures
> 4.630 torr
Which of the following has the highest vapour pressure?
Water
Mercury
Glycerol
Isopentane
The boiling point of water would be highest at:
Murree
Mount Everest
Siachin
Gwadar
Which of the following is false for evaporation?
surface phenomenon
continuous
causes cooling
exothermic
The vapour pressure of water at 100°C is:
55 mm Hg
355 mm Hg
1489 mm Hg
760 mm Hg
The conversion of vapours back to liquid is called:
Crystallization
Evaporation
Vapourization
Condensation
Which of the following has highest volatility?
Ethyl alcohol
Water
Ethylene glycol
Diethyl ether
To maintain the boiling point of water at 110°C, the pressure should be:
Between 200 torr and 760 torr
765 torr
Any pressure value
Between 760 torr and 1200 torr
If we provide very high amount of heat to a liquid its boiling point will
Increase
Decrease
There will be no boiling
Remains constant
Evaporation is designated as a cooling process because of the reason
It is a surface phenomenon
It is exothermic process
All of the above
High energy molecules leave behind the low energy molecules and cause cooling
Vapour pressure of a liquid depends on:
Surface area and temperature only
Volume of the liquid
Humidity of the liquid in the air
Temperature and intermolecular forces
At 1 atm pressure, liquid 1 has a boiling point lower than liquid 2. What can we predict about both liquids?
Liquid 1 has a higher vapour pressure than liquid 2
Liquid 1 has weaker intermolecular forces of attraction than liquid 2
Liquid 1 is more volatile than liquid 2
All of the above
The distillation of a solution under reduced pressure is called:
Fractional distillation
Distillation
Destructive distillation
Vacuum distillation
A pressure cooker reduces cooking time because:
A large flame is used
Heat is uniformly distributed
Vapour pressure of the liquid decreases
The boiling point of water rises
Molar heat of vaporization of water is:
140.6 kJ mol⁻¹
14.6 kJ mol⁻¹
Zero
40.6 kJ mol⁻¹
The rate of evaporation of a liquid does not depend on:
Surface area of the liquid
Temperature
Intermolecular forces
All of these
Which one of the following would cause severe burning?
Boiling water at 90°C
Boiling water at 80°C
Water at 20°C
Steam at 100°C
The boiling point of a liquid is the temperature at which:
The vapour pressure of the liquid is less than the atmospheric pressure
The vapour pressure of the liquid is greater than the atmospheric pressure
The vapour pressure of the liquid is equal to the intermolecular forces of the liquid molecules
The vapour pressure of the liquid is equal to the atmospheric pressure
The strength of hydrogen bonding is:
20 times less than an ionic bond
20 times more than a covalent bond
20 times more than an ionic bond
20 times less than a covalent bond
When ammonia is dissolved in water, the number of hydrogen bonds formed by ammonia is:
Lower alcohols are soluble in water because:
Dipole-induced dipole forces
Low electronegativity difference between C and H
All of the above
Intermolecular hydrogen bonding
The strongest hydrogen bond is:
When two ice cubes are pressed against each other, they stick due to:
Covalent attraction
Ionic bond formation
Metallic bond formation
Hydrogen bond formation
Which of the following can form hydrogen bonding among its molecules more prominently?
CH₃COOH
CHCl₃
All of these
CH₃OH
Hydrogen bonding is involved in:
Solubility
Cleansing action of detergents
Biological molecules
All of the above
When water freezes at 0°C, its density decreases due to:
Change in bond angles
Cubic structure of ice
Change in bond length
Empty space present in the structure of ice
The correct order of boiling points of the given liquids is: (MDCAT 2012)
H₂O > HF > HCl > NH₃
HF > H₂O > HCl > NH₃
HF > H₂O > NH₃ > HCl
H₂O > HF > NH₃ > HCl
At 1489 mmHg, water will boil at: (NUMS 2019)
Ice is less dense than water at: (MDCAT 2014)
In the crystal lattice of ice, each oxygen atom of a water molecule is attached to: (MDCAT 2014)
Two hydrogen atoms
One hydrogen atom
Three hydrogen atoms
Four hydrogen atoms
What is the reason that ice at 0°C occupies more volume than water?
Ionic bonds
Intermolecular forces
Debye forces
Empty spaces in the structure
Water has maximum density at: (NUMS 2019)
The DNA molecule is double-stranded, in which two chains of DNA are twisted around each other by: (MDCAT 2011)
Van der Waals forces
Covalent bonds
Dative bonds
Hydrogen bonds
Which of the following substances exhibits hydrogen bonding? (MDCAT 2017)
In an H-F bond, the electronegativity difference is 2.0. What is the type of this bond? (MDCAT 2019)
π (pi) bond
Non-polar covalent bond
Co-ordinate covalent bond
Polar covalent bond
The boiling point of water is higher than petrol because intermolecular forces in water are: (MDCAT 2011)
Weaker than petrol
The same as in petrol
Negligible
Stronger than petrol
Conduction in metals involves the relatively free movement of: (MDCAT 2017)
Atoms
Molecules
Ions
Electrons
Which type of force is present in gasoline? (MDCAT 2015)
Hydrogen bonding
Dipole-dipole forces
Dipole-induced dipole forces
London dispersion forces
Which hydrogen bond is stronger than others? (MDCAT 2015)
O—H⋯O—H
N—H⋯N—H
N—H⋯O—H
F—H⋯F—H
An intermolecular force of attraction X is relatively stronger than the other intermolecular forces, it stabilizes the α-helix and β-pleated sheet structures of proteins. The double helical structure of DNA is also stabilized by this force of attraction. Identify X. (MDCAT 2019)
Dipole-dipole attraction
Ionic interactions
van der Waals forces
Hydrogen bonding
The helical structure of DNA is also stabilized by: (MDCAT 2019)
Dipole-dipole attraction
Ionic interactions
van der Waals forces
Hydrogen bonding
At higher altitudes, the boiling point of water is less than 100°C due to: (ETEA 2019)
Higher atmospheric pressure
No change in atmospheric pressure
Weak hydrogen bonding
Lower atmospheric pressure
Steam causes severe burns compared to boiling water because: (ETEA 2019)
Absence of hydrogen bonding
Freely moving molecules
Statement is incorrect
High latent heat of vaporization
According to Watson and Crick’s model, the double helix structure of DNA is held together by: (MDCAT 2019)
van der Waals forces
Ionic bonding
Dipole-induced dipole forces
Hydrogen bonding
Which of the following substances exhibits hydrogen bonding? (MDCAT 2019)
SO₂ and CO₂ are both tri-atomic molecules, but the heat of vaporization of SO₂ is greater due to: (MDCAT 2020)
High electronegativity of S
Greater size of SO₂
SO₂ is an ionic molecule
SO₂ is polar, and CO₂ is non-polar
Which of the following has the lowest vapor pressure at 20C? (MDCAT 2021)
Diethyl ether
Carbon tetrachloride
Chlorofoam
Water
Which of the following is not a molecular solid? (MDCAT 2020)
Sulphur
Phosphorus
Carbon dioxide
Bromine
Other Chemistry Topics MCQs
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